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Physics > Thermodynamics > Flashcards

Thermodynamics Flashcards

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1
Q

thermal equilibrium

A

when no heat flows between objects

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2
Q

What changes as a function of temperature

A

length, volume, solubility and conductivity

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3
Q

Length expansion equation

A

ΔL=αLΔT

α = coefficient of linear expansion

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4
Q

Volumetric expansion equation

A

ΔV=βVΔT

β = 3α

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5
Q

isolated systems

A

not capable of exchanging energy or matter with their surroundings

total change in internal energy must be zero

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6
Q

closed systems

A

capable of exchanging energy but not matter with surroundings

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7
Q

Open systems

A

can exchange both matter and energy with the environment

matter can carry energy and can be transferred in the form of heat or work

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8
Q

state functions

A

path independent to get to particular equilibrium state

pressure, density, temperature, volume, enthalpy, internal energy, gibbs free energy, and entropy

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9
Q

process functions

A

depend on the path taken to get from one state to another

work and heat

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10
Q

first law of thermodynamics

A

change in the total internal energy of the system is equal to the amount of energy transferred in the form of heat to the system minus the amount of work transferred in the form of work

ΔU = Q-W

energy cannot be created or destroyed, only exchanged

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11
Q

positive Q

A

heat flows into the system

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12
Q

negative Q

A

heat flows out of the system

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13
Q

positive W

A

work is done by the system (expansion)

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14
Q

negative W

A

work is done on the system (compression)

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15
Q

negative ΔU

A

decreasing temperature

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16
Q

positive ΔU

A

increasing temperature

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17
Q

second law of thermodynamics

A

objects in thermal contact and not in thermal equilibrium will exchange heat energy such that hotter object gives heat to colder object

increase entropy

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18
Q

Heat

A

process by which a quantity of energy is transferred between two objects as a result of a difference in temperature

heat cannot be spontaneously transfer energy from a cooler to a warmer object without work being done on the system

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19
Q

Calorie to Joules

A

1 Cal = 10^3 cal = 4184 J

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20
Q

Conduction

A

transfer of energy between objects through molecular collisions

must have direct physical contact between objects

hotter object transfers some kinetic energy to particles of cooler matter through collisions between the particles of the two materials

ex: touching a hot stove

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21
Q

What are the best heat conductors?

A

metals because metallic bonds contain density of atoms embedded in sea of electrons which facilitates rapid energy transfer

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22
Q

What are the poorest heat conductors?

A

gases because there is so much space between individual molecules which makes energy-transferring collisions occurring infrequently

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23
Q

convection

A

transfer of heat through physical motion of the fluid over the material

only liquids and gases can use this

ex: convection ovens circle hot air inside the oven which causes rapid cooking
ex: using an ice bath to rapidly cool something

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24
Q

Radiation

A

transfer of energy by electromagnetic waves (through a vacuum)

ex: way sun is able to warm the earth

25
Q

specific heat

A

amount of heat energy required to raise one gram of a substance by one degree C/K

changes depending on phase

q=mcΔT

26
Q

specific heat of water

A

1 cal/g*K

27
Q

What happens when you add heat to ice?

A

the heat energy causes water molecules to move away from one another because breaking hydrogen bonds

now the water molecules are held less rigidly in place and have greater degrees of freedom of movement, average PE increases

28
Q

equation for phase change

A

q = mL

q = amount of heat gained or lost
m= mass of substance
L= heat of transformation
29
Q

heat of fusion

A

heat of transformation between solid and liquid (either direction)

30
Q

heat of vaporization

A

heat of transformation between liquid and gas

31
Q

melting

A

solid to liquid

32
Q

freezing

A

liquid to solid

33
Q

condensation

A

gas to liquid

34
Q

evaporation/vaporization

A

liquid to gas

35
Q

sublimation

A

solid to gas

36
Q

deposition

A

gas to solid

37
Q

isobaric

A

pressure held constant

38
Q

isothermic

A

constant temperature

ΔU=0
W=Q

39
Q

isochoric

A

isovolumetric
constant volume
W=0

ΔU=Q

40
Q

adiabatic

A

no heat exchange
Q=0
ΔU= -W

41
Q

entropy

A

measure of spontaneous dispersal of energy at a specific temperature

ΔS = Q/T

entropy increases when energy is distributed into a system at a given temperature

42
Q

the entropy of a system can decrease when?

A

the entropy of surroundings increases by at least as much

because the entropy of the universe must remain constant or increase during all processes

43
Q

1 mole = how many liters at STP

A

22.4L

44
Q

gas constants

A
  1. 0821 atm L/mol K

8. 314 J/mol K

45
Q

Gay Lussac’s Law

A

Pressure is directly proportional to Temperature

P1/T1 = P2/T2

46
Q

Charles’ Law

A

Temperature is directly proportional to volume

V1/T1 = V2/T2

47
Q

Avogadro’s Law

A

volume is proportional to number of moles

V1/n1 = V2/n2

48
Q

Boyles’ Law

A

Pressure is inversely proportional to volume

P1V1 = P2V2

49
Q

Van der Waals equation

A

(P + a(n/v)^2)(V-nb) = nRT

50
Q

Boltzman’s Constant

A

PV = NkbT

kb=n/NR
kb=1/Na(R)
N= nNa (number of moles x avogadro’s number)

kb=1.38x10^-23 J/K

allows us to find ideal gas law focusing on number of molecules

51
Q

internal energy

A

Uint = 3/2PV = 3/2NKbT = 3/2nRT

equal to internal energy

52
Q

changing internal energy

A

ΔU = Q + W

if you are doing work on gas = +W
if the gas is doing work = -W

W = PΔV

53
Q

What is the work done when pressure is constant

A

W = PΔV

54
Q

heat capacity

A

if a certain amount of heat is added, how much will the gas expand

C= Q/ΔT

55
Q

molar heat capacity

A

C = Q/nΔT

when at constant volume
C = 3/2R

when at constant pressure
C=5/2R

56
Q

heat capacity (volume)

A

keeping the volume the same will increase pressure as we add more heat

C = Q/ΔT

no work can be done because no expansion; will heat up

Cv = ΔU/ΔT = 3/2PV/ΔT = 3/2Nkb = 3/2nR

Cv=3/2nR

57
Q

heat capacity (pressure)

A

work can be done on the gas

Cp = Q/ΔT = ΔU-W/ΔT = ΔU-PΔV/ΔT = 3/2nRΔT + PΔV/ΔT = 3/2nRΔT + nRΔT/ΔT = 3/2nR + nR = 5/2 nR

Cp = 5/2nR

58
Q

force equation

A

F = ΔP/ΔT = mΔv/ΔT

Physics (8 decks)

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